A 50.00-mL solution of 0.0729 M chloroacetic acid (K_a = 1.4 $\times$ 10^-3)is titrated with a 0.0181 M solution of NaOH as the titrant.What is the pH of at the equivalence point? (K_w = 1.00 $\times$ 10^-14) A) 7.51 B) 11.65 C) 6.49 D) 11.15 E) 2.85

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Quizplus · Accepted Answer

The equivalence point is when the moles of acid are equal to the moles of base added. At this point, the solution will be neutral, so the pH will be 7.

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